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The heat evolved in the decomposition of 7.647 g of ammonium nitrate can be

measured in a bomb calorimeter. The temperature of the calorimeter, which contains

415 g of water, increases from 18.90 °C to 20.72 °C. The heat capacity of the bomb

calorimeter is 155 J/K. What is ΔH for the reaction, assuming that the specific heat

capacity of the pure water is 4.18 J/g/°C.

Assume you mix 100.0mL of .200M CsOH with 50.0 mL of .400 M HCl ina coffee-cup calorimeter. The following reaction occurs:

CsOH (aq)+ HCl (aq) CsCl(aq) + H2O (l)

The temperature of both solution before mixing was 22.5 *C and it rises to 24.28 *C after the acid-base rxn. What is the enthalpy change for the reaction per mole of CsOH? Assume the densities of the solution are 1.00 g/ml and specific heat of solution is 4.2J/g*k.

PS - The correct answer is Delta H = -56 kJ per mol CsOH

Ni(s) + 4CO(g) <---> Ni(CO)4(g)

ΔHf°(kJ/mol) : Ni(s) = 0, CO(g) = -110.525, Ni(CO)4 = -602.9

S°(J/K·mol) : Ni(s) = 29.87, CO(g) = 197.674, Ni(CO)4 = 410.6

a) Is the reaction product-favoured at 25°C?

b) Is the reaction enthalpy or entropy driven? Explain.

c) What is the value of K at 25°C?

d) At what temperature, in °C, will this reaction become spontaneous?

Please show steps if possible.

Apply Hess’s Law, use the data of the given reaction and data from the data table to calculate the enthalpy change for the formation of nitrogen monoxide from its elements.

(Hint: Which reaction is described with the data: ΔH f H2O(g) = −241.8 kJ / mol )

Pas die Wet van Hess toe, gebruik die data van die gegewe reaksie en data uit die datatabel en bereken die entalpie verandering vir die vorming van stikstofmonoksied vanuit sy elemente.

(Wenk: Watter reaksie word beskryf met die data: ΔH f H2O(g) = −241.8 kJ / mol )

4 NH3 (g) + 5 O2(g) → 4 NO(g) + 6 H2O(g) ΔH rxn = −906.2 kJ

The link to the table is http://boomeria.org/chemtextbook/tableA-6.jpg

Silver nitrate is added to a 25 cm3 sample of hydrochloric acid. A white precipitate of silver chloride is then filtered off. If the dry precipitate weighs 0.3537 g, determine the pH of the hydrochloric acid solution.